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Module 2 (2-6) > Chapter 2 > Flashcards

Chapter 2 Flashcards

1
Q

What is the relative charge on a proton?

A

+1

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2
Q

What is the relative charge on a neutron?

A

0

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3
Q

What is the relative charge on an electron?

A

-1

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4
Q

What is the relative mass on an electron?

A

0.0005

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5
Q

What is the relative mass on a proton?

A

1

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6
Q

What is the relative mass on a neutron

A

1

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7
Q

What holds an atom together?

A

The electrostatic attraction between the positive nucleus and negatively charged electrons orbiting around it is what holds an atom together.

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8
Q

What does the mass number mean?

A

Mass number = number of protons + number of neutrons

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9
Q

How do we calculate the number of protons?

A

Number of protons = mass number - number of neutrons

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10
Q

How are ions formed?

A

formed when atoms either gain or lose electrons, causing them to become charged.

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11
Q

What is a positively charged ion called?

A

cation (lost electrons and has fewer electrons then protons)

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12
Q

What is a negatively charged ion called?

A

Anion (gained electrons and has more electrons then protons)

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13
Q

What is an isotope?

A

Isotopes are atoms of the same element that contain the same number of protons and electrons but a different number of neutrons.

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14
Q

How do the properties of an isotope differ from a the normal element?

A

Isotopes have the same chemical properties but different physical properties.

Isotopes of the same element display the same chemical characteristics -This is because they have the same number of electrons in their outer shells.

Electrons take part in chemical reactions and therefore determine the chemistry of an atom.

The only difference between isotopes is the number of neutrons. Since these are neutral subatomic particles, they only add mass to the atom.

As a result of this, isotopes have different physical properties such as small differences in their mass and density

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15
Q

What is the standard isotope that we use to base all atomic masses on?

A

The carbon-12 isotope.

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16
Q

What is the atomic mass unit and how does it work?

A

Its weird to work in Kg so we created the atomic mass unit (u).

Carbon-12 = exactly 12u

so 1u = 1/12th of an atom of carbon-12.

17
Q

What is the definition of relative isotopic mass?

A

The mass on an isotope relative to 1/12th of the mass of carbon-12.

18
Q

What is the definition of relative atomic mass?

A

The weighted mean mass of an atom of an element relative to 1/12th of the mass of carbon-12.

19
Q

How do you determine relative atomic mass?

A

With a mass spectrometer you work out the percentage abundance.

20
Q

How does a mass spectrometer work?

A

-The sample is vapourised
-The sample is ionised to form positive ions
-The ions are accelerated (Heavy ions move slower / are less deflected)
-The ions are detected as a mass-to-charge ratio, written as m over z (mass of ion/charge on ion)
-Each ion produces a signal, so the larger the signal, the greater the abundance

21
Q

How do you work out the relative atomic mass using the relative abundance?

A

you do the (relative abundance x mass) of all the abundances over 100.

22
Q

What is relative molecular mass?

A

Relative molecular mass is applied to chemicals that have a fixed formula in terms of the number of atoms involved (eg. C2H5OH)

23
Q

What is relative formula mass?

A

Relative formula mass is applied to chemicals that use an empirical formula to represent them (eg. CaCl2)

24
Q

What is a binary compound?

A

Contains two elements only.

in ionic compounds the metal always comes first the second element ends with -ide.

25
Q

What are ionic compounds?

A

Formed from a metal and a non-metal bonded together.

Ionic compounds are electrically neutral; the positive charges equal the negative charges

26
Q

What are polyatomic ions?

A

negative ions made up of more than one type of atom.

27
Q

What is an ionic equation?

A

An ionic equation shows only the ions or other particles taking part in a reaction, and not the spectator ions.

28
Q

What is the charge on ammonium (NH4)?

A

NH4+

29
Q

What is the charge on hydroxide (OH)?

A

OH-

30
Q

What is the charge on nitrate (NO3)?

A

(NO3-)

31
Q

What is the charge on nitrite (NO2)?

A

NO2-

32
Q

What is the charge on hydrogen carbonate (HCO3)?

A

HCO3-

33
Q

What is the charge on permanganate (V11) MnO4?

A

MnO4-

34
Q

What is the charge on carbonate (CO3)?

A

CO32-

35
Q

What is the charge on sulphate (SO4)?

A

SO42-

36
Q

What is the charge on sulphite (SO3)?

A

SO32-

37
Q

What is the charge on dichromate (VI) (Cr2O7)?

A

Cr2O72-

38
Q

What is the charge on phosphate (PO4)?

A

PO43-

Module 2 (2-6) (5 decks)

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